Answer: Rotary, Oscillating, Reciprocating.
Oscillating creates pressure on the walls of the container
Explanation: Molecules are colliding with each other and with the wall of the inside of the container bouncing back and forth in oscillating motion. As they collide, they exert force and fill the container. Hence the Oscillating motion creates pressure from swinging of molecules from wall to wall.
Percent yield = 70%
<h3>Further eplanation
</h3>
Percent yield is the comparison of the amount of product obtained from a reaction with the amount you calculated
General formula:
Percent yield = (Actual yield / theoretical yield )x 100%
An actual yield is the amount of product actually produced by the reaction. A theoretical yield is the amount of product that you calculate from the reaction equation according to the product and reactant coefficients
Reaction
2H₂ (g) + O₂ (g) → 2H₂O (g)
- mass of H₂O (theoretical) :
Answer:
C2H3O3
Explanation:
Empirical formula is the simplest whole number ratio of moles of atoms that you can find in a molecule.
In combustion analysis all Carbon reacts producing CO2 and all hydrogen reacts producing H2O. With the differences in masses we can find the mass of oxygen and their moles:
<em>Moles CO2 = Moles C:</em>
14.08g * (1mol/44.01g) = 0.3199 moles C * (12.01g/mol) = 3.8423g C
<em>Moles H2O:</em>
4.32g H2O * (1mol/18.01g) = 0.2399 moles H2O * (2mol H / 1molH2O) = 0.4797moles H = 0.4797g H
<em>Mass O:</em>
12.01g = Mass O + 3.8423g C + 0.4797g H
Mass O = 7.688g O
<em>Moles O:</em>
7.688g O * (1mol/16g) = 0.48 moles O
The ratio of atoms (Dividing in the moles of C that are the lower number of moles):
O: 0.48moles O / 0.3199 moles C = 1.50
C: 0.3199 moles C / 0.3199 moles C = 1
H: 0.4797 moles H / 0.3199 moles C = 1.50
As empirical formula requires whole numbers:
O: 1.50* 2 = 3
C: 1*2 = 2
H: 1.50*2 = 3
The empirical formula is:
<h3>C2H3O3</h3>
Answer: 1. F
2. F
3. T
4. F
5. T
6. T
Explanation:
I am not sure i'm sorry if it isn't right